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Chapter 7: Problem 93

How many 4\(d\) electrons would be predicted in the ground state for the following elements? a. zirconium b. cadmium c. iridium d. iron

Short Answer

Expert verified
In the ground state, the number of 4\(d\) electrons for the given elements are: a. Zirconium: 2 b. Cadmium: 10 c. Iridium: 10 d. Iron: 0

Step by step solution

01

Find the atomic number of each element

Using the periodic table, find the atomic number (number of protons) for each element. This atomic number is also equal to the number of electrons in the ground state of the elements to make them electrically neutral. a. zirconium (Zr) - 40 b. cadmium (Cd) - 48 c. iridium (Ir) - 77 d. iron (Fe) - 26
02

Write the electron configurations for each element

Write the electron configurations of these elements using the Aufbau principle and Pauli's exclusion principle. The electron configurations will help us identify the total number of 4d electrons in each element: a. Zirconium (Zr): \[1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^2\] b. Cadmium (Cd): \[1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2\] c. Iridium (Ir): \[1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^7\] d. Iron (Fe): \[1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6\]
03

Count the number of 4d electrons for each element

Using the obtained electron configurations, count the number of 4d electrons for each of these elements: a. Zirconium (Zr): 2 electrons in 4d orbital b. Cadmium (Cd): 10 electrons in 4d orbital c. Iridium (Ir): 10 electrons in 4d orbital d. Iron (Fe): 0 electrons in 4d orbital (no 4d electrons) So, in the ground state, the number of 4\(d\) electrons are: a. Zirconium: 2 b. Cadmium: 10 c. Iridium: 10 d. Iron: 0

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Most popular questions from this chapter

Predict some of the properties of element 117 (the symbol is Uus, following conventions proposed by the International Union of Pure and Applied Chemistry, or IUPAC). a. What will be its electron configuration? b. What element will it most resemble chemically? c. What will be the formula of the neutral binary compounds it forms with sodium, magnesium, carbon, and oxygen? d. What oxyanions would you expect Uus to form?

It takes \(7.21 \times 10^{-19} \mathrm{J}\) of energy to remove an electron from an iron atom. What is the maximum wavelength of light that can do this?

The electron affinities of the elements from aluminum to chlorine are \(-44,-120,-74,-200.4,\) and \(-384.7 \mathrm{kJ} / \mathrm{mol}\) respectively. Rationalize the trend in these values.

In the ground state of cadmium, Cd, a. how many electrons have \(\ell=2\) as one of their quantum numbers? b. how many electrons have \(n=4\) as one of their quantum numbers? c. how many electrons have \(m_{\ell}=-1\) as one of their quantum numbers? d. how many electrons hav \(m_{s}=-\frac{1}{2}\) as one of their quantum numbers?

In the second row of the periodic table, Be, N, and Ne all have endothermic (unfavorable) electron affinities, whereas the other second-row elements have exothermic (favorable) electron affinities. Rationalize why Be, N, and Ne have unfavorable electron affinities.
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